Transcript PowerPoint Presentation - Introduction to Atoms & Nuclei

Introduction to Atoms
Section 1 page 102- 108
Some videos…
• http://www.youtube.com/watch?v=caYxr
ueCHiQ
• You might be giants - Elements
History of Atomic Models
• Democritus (~400BC)
– atomos = small, solid, indestructible
particles of different shapes & sizes
– These were just ideas, not truly
science…
• Dalton’s Atomic Theory (1803)
– Billiard Ball Model - small solid sphere
– Developed notion of conservation of
mass and that atoms combine in
specific ratios
History of Atomic
Models
• J.J. Thomson (1904)
– Plum Pudding Model - positive and
negative particles dispersed
throughout the atom
http://www.youtube.com/watch?v=XU8nMKkzbT8
Rutherford
– Nuclear Model
(1910)
– Discovered dense positively charged
nucleus of the atom while working with
alpha particles
• Gold Foil Experiment
History of Atomic Models
• Neils Bohr – (1913)
– Also Solar System Model
– Electrons travel in specific, circular orbits
• Schrodinger & Heisenburg – (1926)
– Quantum Mechanical Model
– Dense nucleus w/ protons & neutrons
– Electrons exist in ‘clouds’ called orbitals w/
specific energy levels
Atomic Theory TIMELINE
Create a timeline showing the
development of the atomic theory
Include the following
- Dates
- Events
- Names
- Illustration for each date
ATOMS
Smallest unit of
matter
An atom has three parts:
Particles
Charges
Location
• Proton
= positive (+) center of nucleus
• Neutron = no charge
center of nucleus
• Electron = negative (-) orbit the nucleus
10/1/2013 Atoms QUIZ 1
Particles
Protons
3._______
Electrons
Charge
1.______
no charge
4. ________
(10 points)
Location
2._______
nucleus
5._______
The Atoms Family was created by Kathleen Crawford, 1994
Presentation developed by Tracy Trimpe, 2006, http://sciencespot.net/
The Atoms Family - Atomic Math
Challenge
Atomic Number
Symbol
Name
Atomic Mass
Atomic number equals the number of ____________
protons or
________________.
electrons
Atomic mass equals the number of ______________
+
protons
_______________.
neutrons
To find the total of neutrons Subtract atomic # from mass
Example: Aluminum 13 protons
27-13 = 14 neutrons
#
Assignment: Finish the rest of the worksheet and turn it in to your
teacher.
10/2/2013 Atoms QUIZ 2
9
F
Fluorine
18.998
(10 points)
1. __________ Atomic #
2. __________ Mass
3. __________ # of protons
4. __________# Neutrons
5. __________# Electrons
Bohr Diagrams
• Find out which period
(row) your element is
in.
• Elements in the 1st
period have one
energy level.
• Elements in the 2nd
period have two
energy levels, and so
on.
Nucleus
1st shell
2nd shell
3rd shell
Bohr Diagrams
C
1) Draw a nucleus with
the element symbol
inside.
2) Carbon is in the 2nd
period, so it has two
energy levels, or
shells.
3) Draw the shells
around the nucleus.
Bohr Diagrams
C
1) Add the electrons.
2) Carbon has 6
electrons.
3) The first shell can
only hold 2
electrons.
Bohr Diagrams
C
1) Since you have 2
electrons already
drawn, you need to
add 4 more.
2) These go in the 2nd
shell.
3) Add one at a time starting on the right
side and going
counter clock-wise.
Bohr
Diagrams
1) Check your work.
C
2) You should have 6
total electrons for
Carbon.
3) Only two electrons
can fit in the 1st shell.
4) The 2nd shell can hold
up to 8 electrons.
5) The 3rd shell can hold
18, but the elements
in the first few
periods only use 8
electrons.
Bohr Diagrams
Try the following
elements on your own:
C
a)
b)
c)
d)
e)
f)
H
He
O
Al
Ne
K
10/3/2013 Bohr Model Quiz 3
(10 points)
Create a Bohr Model for the following elements:
Protons = BLUE
Electrons=RED
Neutron= GREEN
1.
5
2.
10
B
Ne
Boron
10.81
Neon
20.180
Organization of Elements and Families
Periods on the Periodic Table
• Horizontal rows that consist of different
elements
• From left to right the prosperities change in
patterns
– Left = highly active
– Middle = less active
– Right= less active
Families on the Periodic Table
• Elements on the periodic table can be grouped
into FAMILIES bases on their chemical
properties.
• Each family has a specific name to
differentiate it from the other families in the
periodic table.
• Elements in each family
react differently with
other elements.
ALKALI METALS
Brown)
Group 1 Elements:
-Lithium
-Rubidium
-Sodium
-Cesium
-Potassium -Francium
• Silvery Solids
• Low Densities
• Low Melting Points
• Hydrogen is NOT a member,
it is a non-metal
ALKALINE EARTH METALS (dark Green)
The Group 2
Elements
-Beryllium -Magnesium
-Calcium -Strontium
-Barium
-Radium
• Higher melting points
than Alkali Metals
• Reactive, but less than
Alkali metals
• Conduct electricity
TRANSITION METALS (Light Blue)
Groups 3-12 in the
middle
Good conductors of
heat and
electricity.
 Some are used for
jewelry.
 Can bond with
many elements in a
variety of shapes.
BORON FAMILY (Red)
Group 13 Elements
-Boron -Aluminum
-Gallium -Indium
-Thallium
• All are metals except
Boron
• Aluminum is the most
common metal in the
Earth’s crust.
CARBON
FAMILY
(Yellow)
Group 14 Elements
Group 14
Contains metals,
metalloids, and a
non-metal
Carbon (C)
-Carbon
-Silicon
-Germanium -Tin
-Lead
• Silicon is used to make semiconductors for
computers and other electronics .
• Diamond and Graphite are two forms of carbon.
NITROGEN FAMILY (Bright green)
Group 15
Elements
-Nitrogen
-Phosphorus
-Antimony
-Arsenic
-Bismuth
• Almost 80% of the air
we breathe is nitrogen.
• Phosphorus is an
essential ingredient in
healthy teeth and
bones.
OXYGEN FAMILY (Navy)
Group 16 Elements
-Oxygen
-Sulfur
-Selenium -Tellurium
-Polonium
• About 20% of the
Earth’s
atmosphere is
oxygen.
• Sulfuric acid is
one the most used
chemicals in the
world
Halogens (orange)
Group 17
• 7 electrons in
the outer shell
• All are nonmetals
• Very reactive
are often
bonded with
elements from
Group 1
Noble
Gases
(pink)
Group 18 Elements
-Helium -Neon
-Argon
-Krypton
-Xenon
-Radon
• Helium is used to fill balloons.
• Neon signs contain noble gases.
Rare Earth Metals (purple)
• Some are
Radioactive
• The rare earths
are silver,
silvery-white,
or gray metals.
• Conduct
electricity